00 ml of 0.425 m h2so4 solution is required to completely neutralize 23.9 ml of koh solution. what is the molarity of the koh solution

00 mL? I believe that you have erroneously pasted the question here.

Anyway, let us continue computing for the molarity of KOH but i will just use a variable “A” for the volume of H2SO4 solution.

The complete balanced reaction is:

H2SO4  +  2KOH  -->  K2SO4  +  2H2O

We see that 2 moles of KOH is needed for every mole of H2SO4. So calculate the moles of H2SO4.

moles H2SO4 = 0.245 M * (A / 1000) = 2.45x10^-4 A

So the number of moles of KOH is:

moles KOH = 2.45x10^-4 A * 2

moles KOH = 4.90x10^-4 A

So the molarity of KOH is:

Molarity KOH = 4.90x10^-4 A / (0.0239 L)

Molarity KOH = 0.0205 * A

Simply multiply 0.0205 by the correct volume of H2SO4 in ml

120,630,890

step-by-step explanation:

110+10=120,620+10=630,880+10=890

the positions which points up in upward carbon and down in downward carbon are axial

and vice versa holds true for equatorial positions

so the correct answer with labelled diagram will be